Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Question
How do i plug this into my TI-84 calculator. please show me i provided the answer below that im supposed to get.
![**Transcription for Educational Website**
---
**Image Analysis and Transcription**
The image displays a calculation related to the Arrhenius equation, which is used in chemical kinetics to describe the temperature dependence of reaction rates.
1. **Calculator Display:**
The calculator is displaying:
\( 3.54 \times 10^{14} \times \left( \dfrac{-9.15 \times 10^{4}}{8.3145 \times 298} \right) \)
Result: 0
2. **Equation and Calculation Details:**
On the right side, the following information is provided:
**Arrhenius Equation:**
\[
k = A e^{-\frac{E_a}{RT}}
\]
**Given Values:**
- Pre-exponential factor (\(A\)): \(3.54 \times 10^{14}\)
- Activation energy (\(E_a\)): \(-9.15 \times 10^4 \, \text{J/mol}\)
- Universal gas constant (\(R\)): \(8.3145 \, \text{J/mol K}\)
- Temperature (\(T\)): 298 K
**Substituted Equation:**
\[
k = 3.54 \times 10^{14} \times \left( e^{\left(\frac{-9.15 \times 10^{4}}{8.3145 \times 298}\right)} \right)
\]
3. **Expected Result:**
It’s noted that the calculation is supposed to equal \(3.2 \times 10^{-2}\).
---
This analysis provides insight into the application of the Arrhenius equation, highlighting the importance of exponential functions in calculating reaction rates based on temperature.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F08bb2a94-da17-43f2-90ab-4ad444df37b3%2F7c335d9a-dd04-4632-a78a-e96e75224975%2Fnsdz6r_processed.png&w=3840&q=75)
Transcribed Image Text:**Transcription for Educational Website**
---
**Image Analysis and Transcription**
The image displays a calculation related to the Arrhenius equation, which is used in chemical kinetics to describe the temperature dependence of reaction rates.
1. **Calculator Display:**
The calculator is displaying:
\( 3.54 \times 10^{14} \times \left( \dfrac{-9.15 \times 10^{4}}{8.3145 \times 298} \right) \)
Result: 0
2. **Equation and Calculation Details:**
On the right side, the following information is provided:
**Arrhenius Equation:**
\[
k = A e^{-\frac{E_a}{RT}}
\]
**Given Values:**
- Pre-exponential factor (\(A\)): \(3.54 \times 10^{14}\)
- Activation energy (\(E_a\)): \(-9.15 \times 10^4 \, \text{J/mol}\)
- Universal gas constant (\(R\)): \(8.3145 \, \text{J/mol K}\)
- Temperature (\(T\)): 298 K
**Substituted Equation:**
\[
k = 3.54 \times 10^{14} \times \left( e^{\left(\frac{-9.15 \times 10^{4}}{8.3145 \times 298}\right)} \right)
\]
3. **Expected Result:**
It’s noted that the calculation is supposed to equal \(3.2 \times 10^{-2}\).
---
This analysis provides insight into the application of the Arrhenius equation, highlighting the importance of exponential functions in calculating reaction rates based on temperature.
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